(Oligo-)Thiophene Functionalized Tetraazaperopyrenes: Donor

Article pubs.acs.org/joc

(Oligo-)Thiophene Functionalized Tetraazaperopyrenes: Donor− Acceptor Dyes and Ambipolar Organic Semiconductors Lena Hahn,† André Hermannsdorfer,† Benjamin Günther,† Tobias Wesp,† Bastian Bühler,† Ute Zschieschang,‡ Hubert Wadepohl,† Hagen Klauk,‡ and Lutz H. Gade*,† †

Anorganisch-Chemisches Institut, Universität Heidelberg, Im Neuenheimer Feld 270, 69120 Heidelberg, Germany Max Planck Institute for Solid State Research, Heisenbergstr.1, 70569 Stuttgart, Germany

‡

S Supporting Information *

ABSTRACT: Tetraazaperopyrenes (TAPPs) have been functionalized with thiophene and terthiophene units of different architecture resulting in a variety of organic donor−acceptor (D−A) compounds. The influence of the connection of the thiophenes to the TAPP core on their structural, photophysical and electrochemical properties has been studied in detail by a combination of X-ray crystallography, UV−vis and fluorescence spectroscopy as well as cyclic voltammetry, which allowed the establishment of structure−property relationships. The HOMO−LUMO gap is significantly decreased upon substitution of the TAPP core with electron-donating thiophene units, the extent of which is strongly influenced by the orientation of the thiophene units. The latter also crucially directs the molecular packing in the solid. Linkage at the α-position allows both inter- and intramolecular N···S interaction, whereas linkage in the β-position prevents intramolecular N···S interaction, resulting in a less pronounced conjugation of the TAPP core and the thiophene units. The new TAPP derivatives were processed as semiconductors in organic thin-film transistors (TFTs) that show ambipolar behavior. The insight into band gap and structure engineering may open up new possibilities to tailor the electronic properties of TAPP-based materials for certain desired applications.

■

INTRODUCTION

with ambipolar charge-transport that operate under ambient conditions are known to date.21−24 Due to their electron-rich character and resulting electrochemical properties along with their excellent charge-transport properties, thiophene or oligothiophene units are often employed as the electron-donating moieties in D−A systems.25−30 Thiophene moieties attached to electron-poor perylene diimide (PDI) and naphthalene diimide (NDI) units have been the focus of a number of recent studies.27,28,31−48 These types of D−A ensembles have shown potential as materials for ambipolar organic TFTs, organic solar cells and dye-sensitized solar cells.33 We have developed an efficient synthetic route to a class of functional dyes which possess photophysical and redoxchemical properties that are in many respects comparable to those of PDIs. The 1,3,8,10-tetraazaperopyrenes (TAPPs) are readily accessible poly-N-heterocyclic species obtained either from the oxidative coupling of 1,8-diaminonaphthaline or by derivatization of perylenes.49,50 The structure of TAPP is related to the structure of PDI with the two carboximido units at the perylene core being replaced by two fused pyrimidine rings. While PDIs are certainly the most intensely studied class

Ambipolar behavior in organic semiconductors employed in electronic devices may be achieved by appropriate choice of the device architecture by, for example, applying nonsymmetric work-function electrodes,1 electrode surface modifications2 or depositing bilayer/blend semiconductor films.3,4 However, the use of intrinsically ambipolar semiconducting materials would greatly simplify the fabrication of such devices. Donor− acceptor (D−A) conjugated molecules have been of interest for manifold applications in optoelectronics, including donor− acceptor conjugated polymer-based5−11 as well as small molecule-based12−18 ambipolar organic TFTs. Although polymer-based ambipolar organic TFTs tend to display greater electron and hole mobilities than their small molecule-based analogues, the latter have the possible advantage of potentially smaller batch-to-batch variations.19 The frontier orbital energies of the semiconducting material are key parameters determining whether electrons or holes will predominantly be injected into the transistor channel. In order to transport both electrons and holes, the organic semiconductor must usually possess both sufficiently low LUMO levels and at the same time close HOMO and LUMO frontier orbitals with an energy gap in the range of 2.0 eV3,20 which is a significant challenge, explaining why only a few small molecules © 2017 American Chemical Society

Received: September 11, 2017 Published: November 7, 2017 12492

DOI: 10.1021/acs.joc.7b02286 J. Org. Chem. 2017, 82, 12492−12502

Article

The Journal of Organic Chemistry of organic dyes, due to the variety of their applications as for example pigments, biosensors, and as organic semiconductors in organic light emitting diodes as well as in thin film transistors,51−55 the full potential of TAPPs has yet to be explored. TAPPs are characterized by a compact and chemically relatively inert poly-N-heterocyclic core structure which alone has been shown to be a potent electron acceptor unit. Substitution of the TAPP core provides a means of modifying the frontier orbital energy levels and thus of fine-tuning the properties of TAPP-based materials.56,57 These include, inter alia, water-soluble dyes that have been employed as fluorescence markers in cells58 and a variety of TAPP derivatives which have been applied as semiconductors in nchannel organic TFTs.59−61 Here we present the synthesis of a range of thiophene- and oligothiophene-functionalized tetraazaperopyrene derivatives which has given rise to new types of D−A systems. Structure−property relationships are derived from detailed investigations of their molecular packing motifs in the solid as well as their optical, electrochemical and charge-transport properties.

Figure 1. Torsion angles Φ (left) and δ (right) as the key features of the molecular structures.

relatively short N···S distances, leading in all cases to a “headto-head” arrangement in the solid-state structures. This can be attributed to possible N···S interactions, as exemplified by the N···S distances of 2.729 and 2.989 Å in 2 (sum of the Van-derWaals radii being 3.35 Å), which is comparable to other N−S interactions described previously in literature (Figure 2).62,63

■

RESULTS AND DISCUSSION Synthesis of Thiophene-Functionalized Tetraazaperopyrenes. Using a previously reported core-brominated TAPP derivative as the starting material,60 compounds 1−5 were obtained as purple solids in moderate to good yields (53−75%) by Suzuki coupling with the corresponding boronic acid pinacol ester-substituted thiophenes using Pd(dppf)Cl2 as catalyst (Scheme 1). Except for derivative 1, all compounds exhibit Scheme 1. Synthesis of Compounds 1−5 via Suzuki Reaction

Figure 2. Top: Molecular structure of compound 2. Bottom: Interand intramolecular N···S interactions in compound 2. Thermal ellipsoids are drawn at 50% probability level. Hydrogen atoms are omitted for reasons of clarity. Only one of the independent molecules is shown.

good solubility in common organic solvents such as chloroform or THF and thus allowed complete characterization by mass spectrometry, 1H and 13C NMR as well as the investigation of their photophysical and electrochemical properties. Crystal Structures of Compounds 2−5. In a comparative investigation of the solid-state structures of the new TAPP derivatives, single-crystals of the soluble compounds 2−5 suitable for X-ray diffraction were grown from solutions in organic solvents (see SI). As expected, all derivatives have an only slightly distorted TAPP core, represented by the torsion angle Φ (Figure 1), with the distortion of the polycyclic core being slightly more pronounced in the β-thienyl-linked TAPP 5 than in the αlinked thienyl derivatives (with reference to the minimum Φ). In the case of 3, the steric hindrance of the hexyl group prevents the expected planarity, resulting in an enlarged Φ. In contrast to the core twisting, the rotation of the thienyl substituents, represented by the dihedral angle δ, differs greatly, with α-linkage generally leading to a significantly lower out-ofplane rotation. The compounds featuring the latter exhibit

In the case of derivative 3, only two of the thienyl groups are coplanar with respect to the TAPP core, whereas the other two are rotated significantly due to the steric hindrance of the hexyl groups (Figure 3). In contrast, for the β-linked derivatives 4 and 5 no N−S interactions are possible, and the rotation angle of the thienyl units with respect to the TAPP core is thus determined by the sterics of other substituents of the Sheterocycle, as evident in compound 5. A summary of the different distortion and rotation angles is given in Table 1. The packing pattern of compounds 2−4 is similar to most other previously synthesized TAPP derivatives. It is characterized by a slip-stacked face-to-face arrangement of the molecules with π−π plane distances of 3.44−3.47 Å (Table 1). This pattern is exemplified for compound 2 in Figure 4 (top). An exception is the packing pattern of compound 3 that forms trimeric subaggregates which probably result from the orientational effect of the hexyl groups (Figure 4, bottom). 12493


Article

The Journal of Organic Chemistry

Figure 4. Regular packing pattern of compound 2 (top) and aggregation in the form of trimeric units in case of compound 3 (bottom).

TAPP compound 2,9-bis(heptafluoropropyl)-1,3,8,10-tetraazaperopyrene (TAPP-H) recorded in THF are depicted in Figure 5. The thienyl TAPPs exhibit absorption maxima at 493−538 nm, with similar extinction coefficients (log ε ≈ 4.60), that can be attributed to the S1 ← S0 transition. Compared to the parent compound, the absorption maxima of 2−5 exhibit a bathochromic shift, which is the result of the reduced HOMO− LUMO gap, due to the presence of the donor groups. The effect is most pronounced for the derivatives with the smallest interplanar angle δ, and least for 5, in which the rotation out of the TAPP plane prevents an effective conjugation of the thienyl rings and the TAPP core, minimizing the donating effect of the peripheral units. Furthermore, all the TAPPs 2−5 exhibit broadened absorption bands compared to TAPP-H due to the orientational mobility, resulting in a reduced resolution of the vibronic fine structure. The high-energy absorption bands at wavelengths below 400 nm are primarily assigned to excitations localized on the thiophene moieties. The emission spectra of compounds 2−5 were recorded in THF, with emission maxima in the range of 551 to 627 nm. The α-linked compounds 2 and 3 (2848 and 3245 cm−1) exhibit considerably larger Stokes shifts than the β-linked derivatives 4 and 5 (1166 and 2135 cm−1). This indicates that the molecular geometry of the ground state and the excited state differs significantly for α-linked TAPPs, whereas the difference appears to be less pronounced in the β-linked derivatives. With the exception of compound 5 (ϕem = 0.33) the thienyl-substituted TAPPs show intense fluorescence in solution, with fluorescence quantum yields of 62 to 70%. The observed large Stokes shifts are indicative of significant structural differences of the energy minima in the ground state and the first excited state. The absorption and emission maxima as well as the fluorescence quantum yields are listed and related to the interplanar angle δ in Table 2. The frontier orbital energies are key parameters determining whether an organic compound is suitable as a semiconductor in organic electronics and whether electrons or holes will

Figure 3. Molecular structures of 3−5 observed in the solid state. Thermal ellipsoids are drawn at 50% probability level. Hydrogen atoms are omitted for reasons of clarity.

Table 1. Important Geometric Parameters of TAPP Compounds 2−5 Φ [deg]

2 3 4 5

δ [deg]a

min.

max.

min.

max.

rmsd of mean TAPP core plane [Å]

0.9(9) 1.8(4) 0.8(3) 4.7(2)

2.7(9) 9.7(4)

10.2(2) 33.34(8) 17.3(2) 47.83(6)

42.4(2) 57.02(7) 20.2(1) 68.33(5)

0.043, 0.061 0.101, 0.013 0.080 0.108

π−π plane distance [Å] 3.45 3.44 3.47

a

Interplanar angle between thiophene substituent and C10-unit of TAPP core (C1 through C10).

The molecules of 3 have small π−π plane distances of 3.44 Å within the trimeric subaggregate, but large distances of approximately 10 Å between these units. For TAPP derivative 5, the crystals contained solvent molecules in the lattice preventing the comparison of the solid-state structures in terms of the packing pattern and π−π plane distance. Photophysical and Redox-Chemical Properties of the Thienyl-TAPP Compounds 2−5. The UV−vis spectra of compounds 2−5 along with the UV−vis spectrum of the parent 12494


Article


The Kohn−Sham frontier orbitals of 2 are shown in Figure 6 and closely resemble the corresponding MOs of the other thiophene-substituted TAPP derivatives reported in this work. As expected, substitution of the TAPP core with electrondonating thienyl moieties leads to a significant destabilization of the HOMO level compared to the unsubstituted TAPP-H, while the energy of the LUMO, which is localized almost entirely on the TAPP core, is only slightly affected. This results in reduced HOMO−LUMO gaps between 2.51 and 2.00 eV. The observation that the destabilization of the HOMO level is least pronounced for compound 5 is in agreement with a strong torsion of the thiophene units out of the TAPP core plane due to steric repulsion. Experimental estimates of the LUMO levels were obtained for soluble compounds 2−5 by means of cyclic voltammetry (CV) measurements using Fc/Fc+ as an internal standard, setting EHOMO (Fc) = −4.8 eV. The CVs of compounds 2−5 display two reversible reduction waves, indicating the formation of a monoanion and a dianion, respectively (see CV of compound 4 in Figure 7). The LUMO levels deduced from the CV measurements are in good agreement with the calculated values, which has also been observed previously for other TAPP derivatives. The oxidation potentials could not be measured by CV, due to the highly irreversible nature of the oxidation processes. Charge-Transport Properties in Thin-Film Transistors. Core-halogenated TAPP-derivatives have been successfully employed as semiconductors in n-channel organic TFTs that displayed field-effect mobilities of up to 0.17 cm2/(V s).61 As in these previous studies, the electrical properties of compounds 1−5 were studied in TFTs with a bottom-gate, top-contact architecture and a vacuum-deposited semiconductor layer. Electron mobilities (μe, determined in the saturation regime), on/off current ratios (Ion/Ioff), subthreshold swings (SS), and threshold voltages (Vth) were extracted from the measured transfer characteristics. Electron mobilities observed for transistors fabricated with 1−5 as the semiconductor along with the predicted properties and the solid-state-structure characteristics are summarized in Table 4. TFTs based on all five derivatives display n-channel behavior, with electron mobilities ranging from 2 × 10−4 to 6 × 10−3 cm2/(V s). In addition to the n-channel behavior, which is characteristic for most TAPP derivatives reported so far, p-channel behavior was observed for compounds 1, 2 and 4, with hole mobilities in the range of 7 × 10−4 to 0.015 cm2/(V s). This ambipolar transistor behavior is related to the electron-donating thienyl substituents that result in a relatively small HOMO−LUMO gap which allows both electrons and holes to be injected from the gold source and drain contacts into the semiconductor (Table 4). The p-channel behavior is most pronounced for compound 4 with a hole mobility of 0.015 cm2/(V s). In contrast, compounds 3 and 5 display only weak n-channel and no

Figure 5. Top: Absorption spectra of compounds 2−5 and TAPP-H, recorded in THF. Bottom: Absorption and emission bands of 4 recorded in THF.

predominantly be injected into the transistor channel. Therefore, in a first step, the frontier orbital molecular energies and electron affinities of compounds 1−5 were modeled by DFT. The B3LYP functional64−66 and a def2-SVP basis set67 were used for geometry optimization, the molecular orbital energies and the other properties were calculated based on that geometry using a def2-QZVPP basis set.68 The combination of donor−acceptor units in compounds 1− 5 strongly affects the energy levels of the frontier orbitals. The calculated HOMO and LUMO energies of TAPP-H as well as compounds 1−5 are summarized in Table 3.

Table 2. Interplanar Angles and Photophysical Properties of TAPP-Compounds 2−5 in THF δ [deg]a 2 3 4 5 TAPP-H a

min.

max.

10.2(2) 33.34(8) 17.3(2) 47.83(6) −

42.4(2) 57.02(7) 20.2(1) 68.33(5) −

λmax [nm] (log ε) 532 521 538 493 436

(4.59) (4.58) (4.65) (4.65)

λem [nm]

Stokes shift [cm−1]

ϕEm

627 627 574 551 448

2848 3245 1166 2135 938

0.70 0.65 0.62 0.33 0.51

Interplanar angle between thiophene substituent and C10 unit of TAPP core (C1 through C10). 12495


Article

The Journal of Organic Chemistry Table 3. Electrochemical Properties of TAPP-H and Compounds 1−5 EHOMO (DFT) [eV]

ELUMO (DFT) [eV]

ELUMO (CV) [eV]

ΔEHOMO−LUMO [eV]

EA(DFT) [eV]

−5.70 −5.73 −5.73 −5.76 −6.15 −6.61

−3.72 −3.57 −3.57 −3.56 −3.64 −3.66

− −3.76 −3.75 −3.78 −3.70 −

1.98 2.16 2.16 2.20 2.51 2.95

2.77 2.34 2.67 2.67 2.71 2.62

1 2 3a 4 5 TAPP-H a

Hexyl-groups of the thiophene units were simplified to methyl-groups to reduce computational cost (→ 2 = 3!).

chemical properties. In case of 3 we attribute this observation to the trimeric packing pattern described above which is characterized by large distances between the trimer units, preventing efficient charge-transport. In addition, the degree of torsion of the thiophene substituents with respect to the TAPP core, which was found to be most pronounced in the case of compounds 3 and 5, could be a possible reason for the diminished charge transport capability. In contrast, in compounds 2 and 4, the thienyl substituents are almost coplanar with respect to the TAPP core, resulting in a significant interaction of the electron-rich thienyl units and the electron-poor TAPP core, which could explain the ambipolar TFT behavior observed for these compounds. The current− voltage characteristics of organic TFTs fabricated using compound 4 as the semiconductor are shown in Figure 8.

Figure 6. HOMO (left) and LUMO (right) of 2, calculated with B3LYP/def2-SVP//B3LYP/def2-QZVPP. As previously reported50,57,59−61 the substituents in 2- and 9-position have no significant influence in orbital energies, thus C3F7 groups were reduced to CF3 groups to reduce computational cost.

Figure 7. Cyclic voltammogram of compound 4 recorded in THF (sweep rate 50 mV s−1; supporting electrolyte Bu4NPF6, reference SCE).

Table 4. Comparison of Predictive Semiconductor Properties, Solid State Structure Characteristics as Well as Electron and Hole Mobility of Compounds 1−5 π−π distance 1 2 3 4 5

− 3.45 3.44 3.47 −

μe [cm2/(V s)] −3

1 × 10 6 × 10−3 3 × 10−3 1.5 × 10−3 2 × 10−4

Figure 8. Current−voltage characteristics of organic TFTs using compound 4 as the semiconductor, showing n-channel transistor behavior (top) and p-channel transistor behavior (bottom).

μh [cm2/(V s)] 7 × 10−4 4 × 10−4 − 1.5 × 10−2 −

In addition to the intrinsic materials properties the processability and the morphological properties of the TAPP derivatives also have an important influence on the TFT performance. To evaluate the morphology of the vacuumdeposited semiconductor layer, atomic force microscopy (AFM) analysis was conducted; the results are shown in Figure 9. While clearly differing in crystalinity, all four materials give rise to relatively uniform thin film. However, compound 5

measurable p-channel characteristics. The predominantly nchannel behavior of compounds 3 and 5 seems surprising when considering compounds 3 and 2 possess very similar electro12496


Article


Scheme 2. Synthesis of the Terthiophene-Substituted Compounds 8−10

Figure 9. AFM graphs of transistor surfaces of compounds 2 (top left), 3 (top right), 4 (bottom left) and 5 (bottom right).

shows clear formation of aggregated islands which could explain the considerable decrease of mobility in comparison to compounds 1−4. Synthesis of Oligothiophene-Functionalized Tetraazaperopyrenes. In addition to the thiophene-substituted TAPP derivatives 1−5, the terthiophene-substituted compounds 8−10 and 12 were synthesized via two different routes. Reacting the tetrabromo-TAPP with boronic acid pinacol esters 6 and 7 lead to the formation of compounds 8 and 9 in yields of 34% and 59%, respectively.32,69 In the case of 9, the trimethylsilyl substituted boronic pinacol ester was used in order to provide sufficient solubility to ensure the 4-fold substitution. Desilylation of compound 9 with TBAF in THF afforded compound 10 in 72% yield (Scheme 2). For the synthesis of 12 a different approach was chosen. In the first step, compound 4 was reacted with bromine at room temperature, to give the octabrominated compound 11 in a high yield of 82%. Conversion of 11 with 2-thiophene boronic acid pinacol ester resulted in the formation of TAPP derivative 12 with 45% yield (Scheme 3). Photophysical and Electrochemical Properties of Compounds 8, 10 and 12. The UV−vis spectra of compounds 8, 10 and 12 along with the UV−vis spectrum of TAPP-H recorded in THF are depicted in Figure 10 (and the SI). There are significant differences in the absorption spectra of terthiophene-linked compounds 8, 10 and 12 compared to those of compounds 2−5. The absorption spectra display three absorption maxima, two maxima in the range of 330 to 490 nm and a broad low-energy absorption at 662 nm (8), 660 nm (10) and 524 nm (12), respectively. The absorption bands at 483 nm (8), 482 nm (10) and 461 nm (12) are assigned to π* ← π transitions localized on the TAPP-core (λmax(TAPP-H) = 436 nm). The high-energy bands between 330 and 390 nm can be assigned to π* ← π transitions localized on the terthiophene units (λmax (terthiophene) = 354 nm),70 whereas the broad lowenergy absorption band is due to a terthiophene-TAPP charge transfer transition. The absorption maxima of α-linked compounds 8 and 10 are red-shifted compared to the corresponding absorption bands of the β-linked compound 12. This may be explained by the β-

Scheme 3. Synthesis of the TAPP Derivative 12

linkage of the terthiophene unit in compound 12 leading to an increased repulsion of the terthiophene units and causing these substituent units to twist out of the TAPP plane. The result is a less pronounced conjugation of the donor units with the TAPP core. On the other hand, in the case of compounds 8 and 10 it is reasonable to argue that the α-linkage allows intramolecular 12497


Article


Figure 11. Visualization of HOMO (left) and LUMO (right) of compound 12; for clarity reasons the LUMO was visualized only on one of the four terthiophene units.

The two reversible reduction waves indicate the formation of a monoanion and a dianion, respectively (see CV of compound 8 in Figure 10). The LUMO energy levels thus determined via this method were found to be in good agreement with the values calculated by DFT (Table 5). As described for the thienyl-substituted TAPP derivatives 1− 5, compounds 8, 10 and 12 were processed as semiconductor materials in organic TFTs. While compounds 8 and 12 displayed no measurable charge-carrier mobilities, compound 10 was found to show small electron and hole mobilities of 1 × 10−5 cm2/(V s) and 1 × 10−4 cm2/(V s), respectively. We attribute these poor charge-carrier mobilities to the large and rather flexible terthiophene substituents which may prevent close packing in their solid-state structures, resulting in a decrease of intermolecular electronic coupling between neighboring molecules in the bulk material. In the case of compound 10, the substituents will most likely be oriented in a way that allows intramolecular S···N interactions, as observed for compounds 2 and 3, owing to the α-linkage of the thiophene unit to the TAPP core. This would lead to a decrease in flexibility and would therefore explain the slightly better TFT performance compared to compounds 8 and 12. The electrochemical, photophysical as well as semiconducting properties of compounds 8, 10 and 12 are summarized in Table 5.

Figure 10. Top: UV−vis absorption spectra of compounds 8 and 10. Bottom: Cyclic voltammogram of compound 8 recorded in THF (sweep rate 50 mV s−1; supporting electrolyte Bu4NPF6, reference SCE).

nitrogen−sulfur interactions (as observed for compounds 2 and 3), favoring a coplanar orientation of the terthiophene units which results in an effective conjugation of the electrondonating and electron-accepting units. This would also explain the observation that the intensity of the charge transfer band is much greater for compounds 8 and 10 than for compound 12. While TAPP derivatives 2−5 show moderate to strong fluorescence in solution, no fluorescence was observed for compounds 8, 10 and 12. We attribute this to the possibility of photoinduced intramolecular electron transfer (PET) between the donor and acceptor moieties, which has also been described for donor-substituted PDIs in literature.27,28,31,32,34 The clearcut intramolecular donor−acceptor character of these three TAPP derivatives is also illustrated by the distinct spatial separation of the HOMO and LUMO Kohn−Sham orbitals of compound 12 which are displayed in Figure 11. Whereas the HOMO is situated on the terthiophene-units, the LUMO is localized on the TAPP core. The cyclic voltammograms of the terthiophene-substituted TAPPs feature reversible reduction waves while all oxidations were found to be highly irreversible. Thus, the experimental determination of the LUMO levels for compounds 8, 10 and 12 by means of cyclic voltammetry (CV) was carried out using Fc/Fc+ as an internal standard, setting EHOMO(Fc) = −4.8 eV.

■

CONCLUSIONS We have presented a first study on the impact of donor functionalization of the tetraazaperopyrene core on the properties of such donor−acceptor based organic functional materials. It was demonstrated that the HOMO−LUMO gap is significantly decreased by substitution of the TAPP core with donor units resulting in a remarkable bathochromic shift of the TAPP-centered absorption maxima relative to that of the unsubstituted parent compound. The decrease of the HOMO− LUMO gap and therefore the influence on the photophysical and electrochemical properties was found to depend strongly on the type of linkage between the thiophene unit and the TAPP core. For derivatives with linkages in the α-position both intra- and intermolecular nitrogen sulfur interactions were observed in the solid state structure leading to an almost coplanar orientation of the thiophene unit with respect to the TAPP core. In the case of β-linkage only intermolecular N−S interactions were observed, and the thiophene units are tilted out of the TAPP plane. Finally, the TAPP-derivatives were employed in organic TFTs. While the terthiophenyl-coupled TAPPs display no or only low n- and p-channel mobility, the 12498


Article

The Journal of Organic Chemistry Table 5. Electrochemical, Photophysical as Well as Electron and Hole Mobility of Compounds 8, 10 and 12

8 10 12

ELUMO (CV) [eV]

ELUMO (DFT) [eV]

EHOMO (DFT) [eV]

gap (DFT) [eV]

λ1(max) [nm]

λ2(max) [nm]

λ3(max) [nm]

μe [cm2/(V s)]

μh [cm2/(V s)]

−3.80 −3.96 −3.83

−3.52 −3.67 −3.54

−5.36 −5.36 −5.51

1.84 1.69 1.97

347 360 332

483 482 461

662 660 524

− 1 × 10−5 −

− 1 × 10−4 −

as a violet solid (108 mg, 53%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, CD2Cl2 295 K) δ (ppm) = 9.93 (s, 4 H, H-3), 7.76 (d,3JHH = 5.2 Hz,4 H, H-11), 7.30 (d, 3JHH = 5.3 Hz, 4 H, H-10), 2.82 (t, 3JHH = 7.8 Hz 8 H, H-12), 1.69 (quint. 3JHH = 7.1 Hz, 8 H, H-13), 1.19 (quint, 3 JHH = 7.3 Hz, 8 H, H-14), 1.06 (m, 16 H, H-15/16), 0.64 (m; 12H, H-17) 13C NMR (150.90 MHz, CD2Cl2 295 K) δ (ppm) = 153.9 (C7), 153.6 (C-1), 143.4 (C-9), 135.6 (C-2), 132.6 (C-3), 131.6 (C-8), 129.3 (C-10), 127.4 (C-11), 126.6 (C-4), 120.6 (C-5), 117.4 (C-6), 31.7 (C-15), 31.0 (C-13), 30.0 (C-12), 29.3 (C-14), 22.6 (C-16), 14.1 (C-17) perfluorinated carbon atoms were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, CD2Cl2, 295 K) δ (ppm) = −81.12 (t, 3JFF = 9.1 Hz, 6 F, CF3), −113.12 (m, 4 F, CF2), −125.07 (m, 4 F, CF2). HRMS (MALDI−-TOF) calcd. for C68H64F14N4S4 [M]−: 1330.3790, found 1330.3759. Preparation of Compound 4. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetraazaperopyrene (100 mg, 0.10 mmol), 3-thienyl boronic acid (102 mg, 0.80 mmol), PdCl 2 (dppf) (30 mg, 0.04 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 10 mL of toluene and 10 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature, the aqueous layer was extracted three times with chloroform (30 mL). The combined organic layer was dried over MgSO4, the solvent was removed under vacuum and the obtained solid was washed with methanol and pentane to obtain 4 as a blue solid (75 mg, 75%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, THF-d8, 295 K) δ (ppm) = 10.47 (s, 4 H, H-3), 8.87 (dd,3JHH = 3.0 Hz, 4JHH = 1.3 Hz, 4 H, H-9), 8.38 (dd, 3JHH = 5.1 Hz, 4JHH = 1.3 Hz, 4 H, H-11), 7.73 (dd, 3JHH = 5.1 Hz, 4JHH = 3.0 Hz, 4 H, H-10). 13C NMR (150.90 MHz, THF-d8, 323 K) δ (ppm) = 153.8 (C-1), 138.2 (C-8), 135.5 (C-2), 131.0 (C-3), 130.2 (C-11), 128.6 (C-4), 128.0 (C9), 125.7 (C-10), 120.6 (C-5), 118.5 (C-6) perfluorinated carbon atoms and C-7 were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, THF-d8, 295 K) δ (ppm) = −81.09 (t, 3JFF = 9.1 Hz, 6 F, CF3), −113.81 (m, 4 F, CF2), −126.10 (m, 4 F, CF2). HRMS (MALDI+-TOF) calcd. for C44H17F14N4S4 [M + H]+•: 995.0112, found 995.0149. Preparation of Compound 5. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetraazaperopyrene (150 mg, 0.15 mmol), 4-methylthiophene-3boronic acid pinacol ester (274 mg, 1.22 mmol), PdCl2(dppf) (45 mg, 0.06 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 15 mL of toluene and 15 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature, the aqueous layer was extracted three times with chloroform (30 mL). The combined organic layer was dried over MgSO4, the solvent was removed under vacuum and the obtained solid was washed with methanol. Further purification by column chromatography (silica, CHCl3:PE 1:1) afforded 5 as a violet solid (108 mg, 53%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, CD2Cl2, 295 K) δ (ppm) = 9.93 (s, 4 H, H-3), 7.81 (d,3JHH = 3.2 Hz, 4 H, H-9), 7.32−7.31 (m, 4 H, H11), 2.32 (d, 4JHH = 0.6 Hz, 12 H, H-12). 13C NMR (150.90 MHz, CD2Cl2, 295 K) δ (ppm) = 153.9 (C-1), 139.1 (C-8), 138.7 (C-10), 137.8 (C-2), 132.8 (C-3), 127.3 (C-9), 127.2 (C-4), 122.4 (C-11), 121.0 (C-5), 117.6 (C-6), 15.7 (C-12) perfluorinated carbon atoms and C-7 were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, CD2Cl2, 295 K) δ (ppm) = −80.48 (t, 3JFF = 9.3 Hz, 6 F, CF3), −113.44 (m, 4 F, CF2), −125.34 (m, 4 F, CF2). HRMS (MALDI−-TOF) calcd. for C48H24F14N4S4 [M]−: 1050.0660, found 1050.0655.

monothienyl derivatives exhibit moderate charge-carrier mobilities and in some cases even ambipolar behavior.

■

EXPERIMENTAL SECTION

The syntheses were performed under dried argon in standard Schlenk glassware, which was flame-dried prior to use. Solvents were dried according to standard procedures. The 1H and 13C NMR spectra were recorded with Bruker AVANCE 400 and 600II+ spectrometers equipped with variable-temperature units. 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10-tetraazaperopyrene (II) TAPP-Br was synthesized according to the literature procedures.60 All other starting materials were obtained commercially and used without further purification. Preparation of Compound 1. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetra-azaperopyrene (100 mg, 0.10 mmol), 2-thienyl boronic acid (102 mg, 0.80 mmol), PdCl 2 (dppf) (30 mg, 0.04 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 10 mL of toluene and 10 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature, the solvent was removed in vacuo and the obtained solid was washed with water, methanol and pentane to give 1 as a blue solid (59 mg, 60%) which was practically insoluble in all organic solvents and therefore could not be characterized by NMR spectroscopy. mp > 300 °C (decomposition). HRMS (MALDI−-TOF) calcd. for C44H16F14N4S4 [M]−: 994.0034, found 994.0029. Preparation of Compound 2. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetraazaperopyrene (150 mg, 0.15 mmol), 3-methylthiophene-2boronic acid pinacol ester (274 mg, 1.22 mmol), PdCl2(dppf) (45 mg, 0.06 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 15 mL of toluene and 15 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature, the aqueous layer was extracted three times with chloroform (30 mL). The combined organic layer was dried over MgSO4, the solvent was removed under vacuum and the obtained solid was washed with methanol and pentane to give 2 as a violet solid (120 mg, 74%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, CD2Cl2 295 K) δ (ppm) = 9.97 (s, 4 H, H-3), 7.76 (d,3JHH = 5.2 Hz,4 H, H-11), 7.26 (d, 3JHH = 5.2 Hz, 4 H, H-10), 2.54 (s, 12 H, H-12). 13C NMR (150.90 MHz, CD2Cl2 295 K) δ (ppm) = 153.7 (C-1), 138.7 (C-9), 135.2 (C-2), 133.1 (C-3), 132.2 (C-8), 131.2 (C-10), 127.7 (C-11), 127.0 (C-4), 120.7 (C-5), 16.6 (C-12) perfluorinated carbon atoms and C-7 were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, CD2Cl2, 295 K) δ (ppm) = −81.51 (t, 3JFF = 9.3 Hz, 6 F, CF3), −113.59 (m, 4 F, CF2), −125.36 (m, 4 F, CF2). HRMS (MALDI−TOF) calcd. for C48H24F14N4S4 [M]−: 1050.0660, found 1050.0653. Preparation of Compound 3. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetraazaperopyrene (150 mg, 0.15 mmol), 3-hexylthiophene-2-boronic acid pinacol ester (360 mg, 1.22 mmol), PdCl2(dppf) (45 mg, 0.06 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 15 mL of toluene and 15 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature, the aqueous layer was extracted three times with chloroform (30 mL). The combined organic layer was dried over MgSO4, the solvent was removed under vacuum and the obtained solid was washed with methanol. Further purification by column chromatography (silica, PE:EE 30:1) afforded 3 12499


Article

The Journal of Organic Chemistry Preparation of Compound 8. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetraazaperopyrene (100 mg, 0.10 mmol), boronic acid pinacol ester 6 (395 mg, 9.17 mmol), PdCl2(dppf) (30 mg, 0.04 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 10 mL of toluene and 10 mL aqueous Cs2CO3 solution (2 M) the suspension was heated to 105 °C for 3 days. The mixture was allowed to cool to room temperature and extracted with CHCl3 (3 × 50 mL). The combined organic layers were washed with water (3 × 50 mL), dried over anhydrous magnesium sulfate and filtered. The solvent was removed under reduced pressure and the crude product was purified by column chromatography (silica, PE:EE 10:1) to give the product as a dark green solid (64.6 mg, 34.4 μmol, 34%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, CDCl3, 295 K) δ (ppm) = 10.2 (s, 4H), 8.50 (s, 4H, H4 thienyl), 6.66 (s, 4H), 6.63 (s, 4H), 2.46 (s, 24H), 2.28 (s, 12H), 2.27 (s, 12H). 13C NMR (150.90 MHz, CDCl3, 295 K) δ (ppm) = 151.9 (C-1), 139.4 (C-10), 135.7 (C 8), 135.6 (C-12), 135.5 (C-11), 135.3 (C-2), 135.0 (C-15), 133.3 (C-18), 133.1 (C-22), 133.0 (C-19), 132.2 (C-9), 130.4 (C-13), 127.5 (C-21), 127.2 (C 14), 126.5 (C-3), 126.4 (C-4), 119.5 (C-5), 117.6 (C-6), 15.3 (C-23), 15.3 (C20), 14.2 (C-17), 13.9 (C-16), perfluorinated carbon atoms and C-7 were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, CDCl3, 295 K) δ (ppm) = −80.10 (t, 3JFF = 9.0 Hz, 6 F, CF3), −113.48 (m, 4 F, CF2), −125.36 (m, 4 F, CF2). HRMS (MALDI−TOF) calcd. for C92H64F14N4S12 [M]−: 1874.1556, found 1874.1580. Preparation of Compound 9. A flame-dried Schlenk flask was charged with 2,9-Bisheptafluoropropyl-4,7,11,14-tetrabromo-1,3,8,10tetraazaperopyrene (110 mg, 0.11 mmol), boronic acid pinacol ester 7 (508 mg, 1.1 mmol), PdCl2(dppf) (33 mg, 0.044 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 10 mL of toluene and 10 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature; the aqueous layer was extracted three times with chloroform (30 mL). The combined organic layer was dried over MgSO4, the solvent was removed under vacuum and the obtained crude product was purified by column chromatography (silica, PE:CHCl3 10:1) to obtain 9 as dark green solid (147 mg, 59%) mp > 300 °C (dec.). 1H NMR (600.13 MHz, CDCl3, 295 K) δ (ppm) = 10.02 (s, 4 H, H-3), 8.62 (s, 4 H, H-9), 7.36 (d, 3JHH = 3.2 Hz, 4 H, H-14/H-19), 7.29 (d, 3JHH = 3.2 Hz, 4 H, H-14/19), 7.23−7.20 (m, 8 H, H-13/18), 0.37−0.35 (m, 72 H, TMS). 13C NMR (150.90 MHz, CDCl3, 295 K) δ (ppm) = 152.0 (C-1), 143.2 (C-15/20), 142.7 (C12/13), 141.5 (C-15/20), 140.3 (C-12/13), 137.2 (C-10/11), 135.9 (C-10/11), 134.7 (C-13/18), 134.6 (C-13/18), 133.1 (C-9), 132.9 (C-8), 132.8 (C-2), 129.4 (C-14/19), 128.5 (C-14/19), 126.9 (C-4), 126.7 (C-3), 119.9 (C-5), 117.6 (C-6), 0.35 (TMS), 0.29 (TMS), perfluorinated carbon atoms and C-7 were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, CDCl3, 295 K) δ (ppm) = −81.02 (t, 3JFF = 9.1 Hz, 6 F, CF3), −113.49 (m, 4 F, CF2), −125.95 (m, 4 F, CF2). HRMS (MALDI−-TOF) calcd. for C100H96F14N4S12Si8 [M]−: 2226.2214, found 2226.2209. Preparation of Compound 10. In a flame-dried Schlenk flask compound 9 (80 mg, 0.037 mmol) was dissolved in 15 mL of THF and TBAF (1 M in THF, 0.78 mL, 0.78 mmol) was added dropwise. After stirring at room temperature for 2 h, 20 mL of water were added. The aqueous phase was extracted three times with chloroform (150 mL). The combined organic layer was dried over MgSO4, after filtration the solvent was removed in vacuo. The crude product was thus washed three times with both methanol and pentane to obtain 10 as a green solid (21 mg, 72%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, THF-d8, 333 K) δ (ppm) = 10.70 (s, 4 H, H-3), 8.75 (s, 4 H, H9),7.48 (m, 8 H, H-15/20), 7.34 (m, 4 H, H-14/19), 7.30 (m, 4 H, H14/19), 7.11 (m, 8 H, H-13/18). The low solubility of the compound precluded the recording of 13C NMR data. 19F NMR (376.27 MHz, THF-d8, 295 K) δ (ppm) = −81.01 (t, 3JFF = 8.9 Hz, 6 F, CF3), −113.60 (m, 4 F, CF2), −126.17 (m, 4 F, CF2). HRMS (MALDI−TOF) calcd. for C76H32F14N4S12 [M]−: 1649.9051, found 1649.9046. Preparation of Compound 11. A flame-dried Schlenk flask was charged with compound 4 (200 mg, 0.02 mmol). After the addition of 20 mL of THF bromine (0.13 mL, 0.24 mmol) was added and the

reaction mixture was stirred for 24 h at room temperature. After removal of the solvent the crude product was purified by means of column chromatography (silica, CHCl3:PE 3:2). The product 11 was thus obtained as a red solid (266 mg, 82%). mp > 300 °C (dec.). 1H NMR (600.13 MHz, CDCl3) δ (ppm) = 10.13 (s, 4 H, H-3), 7.70 (s, 4 H, H-8). 13C NMR (150.9 MHz, CDCl3) δ (ppm) = 153.0 (C-1), 137.3 (C-9), 134.1 (C-2), 133.8 (C-10), 133.0 (C-3), 126.9 (C-4), 120.9 (C-5), 117.5 (C-6), 112.4 (C-8/11), 111.4 (C-8/11). 19F NMR (376.27 MHz, CD3Cl, 295 K) δ (ppm) = −81.04 (t, 3JFF = 9.0 Hz, 6 F, CF3), −113.1 (m, 4 F, CF2), −125.3 (m, 4 F, CF2). HRMS (MALDI−TOF) calcd. for C44H879Br481Br4F14N4S4 [M]−: 1625.2793, found 1625.2788. Preparation of Compound 12. A flame-dried Schlenk flask was charged with compound 11 (50 mg, 0.03 mmol), 2-thienyl boronic acid (102 mg, 0.80 mmol), Pd(PPh3)2Cl2 (12 mg, 0.017 mmol), and cetyltrimethylammonium bromide (2 mg). After the addition of 10 mL of toluene and 10 mL of aqueous K2CO3 solution (1 M) the suspension was heated to 105 °C for 2 days. The reaction mixture was allowed to cool to room temperature, the aqueous layer was extracted three times with chloroform (30 mL). The combined organic layer was dried over MgSO4, the solvent was removed under vacuum and the crude product was purified by column chromatography (silica PE:CHCl3:Toluene 2:1:1) to obtain 12 as a dark violet solid (37 mg, 45%) mp > 300 °C (dec.). 1H NMR (600.13 MHz, THF-d8, 295 K) δ (ppm) = 10.21 (s, 4 H, H-3), 7.76 (s, 4 H, H-14), 7.42 (dd, 3JHH = 5.1 Hz, 4JHH = 1.0 Hz, 4 H, H-19), 7.40 (dd, 3JHH = 3.6 Hz, 4JHH = 1.0 Hz, 4 H, H-17), 7.10−7.11 (m, 8 H, H-8/H-18), 7.03 (dd, 3JHH = 5.1 Hz, 4JHH = 1.0 Hz, 4 H, H-10), 6.78 (dd, 3JHH = 5.0 Hz, 3JHH = 3.8 Hz, 4 H, H-9). 13C NMR (150.90 MHz, THF-d8, 295 K) δ (ppm) = 154.2 (C-1), 137.3 (C-16), 137.1 (C-13), 136.0 (C-15), 135.2 (C-12), 135.1 (C-12), 134.8 (C-3), 129.0 (C-14), 128.7 (C-18), 128.0 (C-4), 127.7 (C-9), 127.3 (C-8), 126.8 (C-10), 125.8 (C-19), 124.8 (C-17), 121.6 (C-5), 117.9 (C-6) perfluorinated carbon atoms and C-7 were not detected at the attainable S/N ratio. 19F NMR (376.27 MHz, THF-d8, 295 K) δ (ppm) = −82.93 (t, 3JFF = 8.9 Hz, 6 F, CF3), −113.35 (m, 4 F, CF2), −127.72 (m, 4 F, CF2). HRMS (MALDI−TOF) calcd. for C76H32F14N4S12 [M]−: 1649.9052, found 1649.9048.

■

ASSOCIATED CONTENT

S Supporting Information *

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acs.joc.7b02286. NMR, Absorption, Fluorescence spectra, DFT modeling (PDF) X-ray diffraction studies of compounds 2−5 and 11 (CIF) Coordinates of the DFT modeled structures (XYZ)

■

AUTHOR INFORMATION

Corresponding Author

*E-mail: [email protected]. ORCID

Lutz H. Gade: 0000-0002-7107-8169 Notes

The authors declare no competing financial interest.

■

ACKNOWLEDGMENTS We gratefully acknowledge support by the Deutsche Forschungsgemeinschaft (DFG, Sonderforschungsbereich SFB 1249, TP A2 and TP C1).

■

REFERENCES

(1) Rost, C.; Gundlach, D. J.; Karg, S.; Rieß, W. J. Appl. Phys. 2004, 95, 5782−5787.

12500


Article


(32) Fischer, M. K. R.; Kaiser, T. E.; Würthner, F.; Bäuerle, P. J. Mater. Chem. 2009, 19, 1129−1141. (33) Segura, J. L.; Herrera, H.; Bäuerle, P. J. Mater. Chem. 2012, 22, 8717−8733. (34) Wonneberger, H.; Ma, C.-Q.; Gatys, M. A.; Li, C.; Bäuerle, P.; Müllen, K. J. Phys. Chem. B 2010, 114, 14343−14347. (35) Zhan, X.; Tan, Z.; Domercq, B.; An, Z.; Zhang, X.; Barlow, S.; Li, Y.; Zhu, D.; Kippelen, B.; Marder, S. R. J. Am. Chem. Soc. 2007, 129, 7246−7247. (36) Zhang, X.; Lu, Z.; Ye, L.; Zhan, C.; Hou, J.; Zhang, S.; Jiang, B.; Zhao, Y.; Huang, J.; Zhang, S.; Liu, Y.; Qiang, S.; Yunqi, L.; Yao, J. Adv. Mater. 2013, 25, 5791−5797. (37) Zhang, Q.; Cirpan, A.; Russell, T.; Emrick, T. Macromolecules 2009, 42, 1079−1082. (38) Zhou, E.; Cong, J.; Wie, Q.; Tajima, K.; Yang, C.; Hashimoto, K. Angew. Chem., Int. Ed. 2011, 50, 2799−2803. (39) Choi, H.; Paek, S.; Song, J.; Kim, C.; Cho, N.; Ko, J. Chem. Commun. 2011, 47, 5509−5511. (40) Huang, J.; Wu, Y.; Fu, H.; Zhan, X.; Yao, J.; Barlow, S.; Marder, S. R. J. Phys. Chem. A 2009, 113, 5039−5046. (41) Yuan, Z.; Xiao, Y.; Yang, Y.; Xiong, T. Macromolecules 2011, 44, 1788−1791. (42) Fang, K.; Huang, Y.; Chang, G.; Yang, J.; Shen, Y.; Ye, X. Macromol. Res. 2015, 23, 545−551. (43) Schwartz, P.-O.; Biniek, L.; Zaborova, E.; Heinrich, B.; Brinkmann, M.; Leclerc, N.; Méry, S. J. Am. Chem. Soc. 2014, 136, 5981−5992. (44) Deng, P.; Wu, B.; Lei, Y.; Zhou, D.; Ho, C. H. Y.; Zhu, F.; Ong, B. S. Dyes Pigm. 2017, 146, 20−26. (45) Cremer, J.; Mena-Osteritz, E.; Pschierer, N. G.; Müllen, K.; Bäuerle, P. Org. Biomol. Chem. 2005, 3, 985−995. (46) Zhang, C.; Zhao, G.; Zeng, W.; Tian, K.; Dong, H.; Hu, W.; Qin, J.; Yang, C. Org. Electron. 2015, 16, 101−108. (47) Cremer, J.; Bäuerle, P. Eur. J. Org. Chem. 2005, 17, 3715−3723. (48) Usta, H.; Facchetti, A.; Marks, T. J. Acc. Chem. Res. 2011, 44, 501−510. (49) Riehm, T.; De Paoli, G.; Konradsson, A. E.; De Cola, L.; Wadepohl, H.; Gade, L. H. Chem. - Eur. J. 2007, 13, 7317−7329. (50) Martens, S. C.; Riehm, T.; Geib, S.; Wadepohl, H.; Gade, L. H. J. Org. Chem. 2011, 76, 609−617. (51) Würthner, F.; Saha-Möller, C. R.; Fimmel, B.; Ogi, S.; Leowanawat, P.; Schmidt, D. Chem. Rev. 2016, 116, 962−1052. (52) Würthner, F.; Stolte, M. Chem. Commun. 2011, 47, 5109−5115. (53) Anthony, J. E.; Facchetti, A.; Heeney, M.; Marder, S. R.; Zhan, X. Adv. Mater. 2010, 22, 3876−3892. (54) Würthner, F. Chem. Commun. 2004, 1564−1579. (55) Selected references: (a) Laquindanum, J. G.; Katz, H. E.; Dodabalapur, A.; Lovinger, A. J. J. Am. Chem. Soc. 1996, 118, 11331. (b) Lee, S. K.; Zu, Y.; Herrmann, A.; Geerts, Y.; Müllen, K.; Bard, A. J. J. Am. Chem. Soc. 1999, 121, 3513. (c) Quante, H.; Müllen, K. Angew. Chem., Int. Ed. Engl. 1995, 34, 1323. (d) Schmidt-Mende, L.; Fechtenkötter, A.; Müllen, K.; Moons, E.; Friend, R. H.; MacKenzie, J. D. Science 2001, 293, 1119. (e) Ahrens, M. J.; Fuller, M. J.; Wasielewski, M. R. Chem. Mater. 2003, 15, 2684. (f) Qu, J.; Kohl, C.; Pottek, M.; Müllen, K. Angew. Chem., Int. Ed. 2004, 43, 1528−1521. (g) Jones, B. A.; Ahrens, M. J.; Yoon, M.-H.; Facchetti, A.; Marks, T. J.; Wasielewski, M. R. Angew. Chem., Int. Ed. 2004, 43, 6363. (h) Zhan, X.; Tan, Z. A.; Domercq, B.; An, Z.; Zhang, X.; Barlow, S.; Li, Y.; Zhu, D.; Kippelen, B.; Marder, S. R. J. Am. Chem. Soc. 2007, 129, 7246. (i) Franceschin, M.; Pascucci, E.; Alvino, A.; D’Ambrosio, D.; Bianco, A.; Ortaggi, G.; Savino, M. Bioorg. Med. Chem. Lett. 2007, 17, 2515− 2522. (j) Tan, Z. A.; Zhou, E. J.; Zhan, X. W.; Wang, X.; Li, Y. F.; Barlow, S.; Marder, S. R. Appl. Phys. Lett. 2008, 93, 073309. (k) Li, Y.; Tan, L.; Wang, Z.; Qian, H.; Shi, Y.; Hu, W. Org. Lett. 2008, 10, 529− 532. (l) Liu, C.; Liu, Z.; Lemke, H. T.; Tsao, H. N.; Naber, R. C. G.; Li, Y.; Banger, K.; Müllen, K.; Nielsen, M. M.; Sirringhaus, H. Chem. Mater. 2010, 22, 2120. (m) Gsänger, M.; Oh, J. H.; Könemann, M.; Höffken, H. W.; Krause, A.-M.; Bao, Z.; Würthner, F. Angew. Chem.,

(2) Baeg, K.-J.; Kim, J.; Khim, D.; Caironi, M.; Kim, D.-Y.; You, I.-K.; Quinn, J. R.; Facchetti, A.; Noh, Y.-Y. ACS Appl. Mater. Interfaces 2011, 3, 3205−3214. (3) Cornil, J.; Brédas, J.-L.; Zaumseil, J.; Sirringhaus, H. Adv. Mater. 2007, 19, 1791−1799. (4) Xu, X.; Xiao, T.; Gu, X.; Yang, X.; Kershaw, S. V.; Zhao, N.; Xu, J.; Miao, Q. ACS Appl. Mater. Interfaces 2015, 7, 28019−28026. (5) Kim, F. S.; Guo, X.; Watson, M. D.; Jenekhe, S. A. Adv. Mater. 2010, 22, 478−482. (6) Stalder, R.; Puniredd, S. R.; Hansen, M. R.; Koldemir, U.; Grand, C.; Zajaczkowski, W.; Müllen, K.; Pisula, W.; Reynolds, J. R. Chem. Mater. 2016, 28, 1286−1297. (7) Chaing, C.-J.; Chen, J.-C.; Kuo, Y.-J.; Tsao, H.-Y.; Wu, K.-Y.; Wang, C.-L. RSC Adv. 2016, 6, 8628−8638. (8) Gsänger, M.; Bialas, D.; Huang, L.; Stolte, M.; Würthner, F. Adv. Mater. 2016, 28, 3615−3645. (9) Kan, J.; Chen, Y.; Qi, D.; Liu, Y.; Jiang, J. Adv. Mater. 2012, 24, 1755−1758. (10) Khim, D.; Cheon, Y. R.; Xu, Y.; Park, W.-T.; Kwon, S.-K.; Noh, Y.-Y.; Kim, Y.-H. Chem. Mater. 2016, 28, 2287−2294. (11) Steckler, T. T.; Zhang, X.; Hwang, J.; Honeyager, R.; Ohira, S.; Zhang, X.-H.; Grant, A.; Ellinger, S.; Odom, S. A.; Sweat, D.; Tanner, D. B.; Rinzler, A. G.; Barlow, S.; Brédas, J.-L.; Kippelen, B.; Marder, S. R.; Reynolds, J. R. J. Am. Chem. Soc. 2009, 131, 2824−2826. (12) Anthopoulos, T. D.; Tanase, C.; Setayesh, S.; Meijer, E. J.; Hummelen, J. C.; Blom, P. W. M.; de Leeuw, D. M. Adv. Mater. 2004, 16, 2174−2179. (13) Chesterfield, R. J.; Newman, C. R.; Pappenfus, T. M.; Ewbank, P. C.; Haukaas, M. H.; Mann, K. R.; Miller, L. L.; Frisbie, C. D. Adv. Mater. 2003, 15, 1278−1282. (14) Kang, W.; Jung, M.; Cha, W.; Jang, S.; Yoon, Y.; Kim, H.; Son, H. J.; Lee, D.-K.; Kim, B.; Cho, J. H. ACS Appl. Mater. Interfaces 2014, 6, 6589−6597. (15) Lin, G.; Qin, Y.; Zhang, J.; Guan, Y.-S.; Xu, H.; Xu, W.; Zhu, D. J. Mater. Chem. C 2016, 4, 4470−4477. (16) Mei, J.; Diao, Y.; Appleton, A. L.; Fang, L.; Bao, Z. J. Am. Chem. Soc. 2013, 135, 6724−6746. (17) Pitayatanakul, O.; Higashino, T.; Kadoya, T.; Tanaka, M.; Kojima, H.; Ashizawa, M.; Kawamoto, T.; Matsumoto, H.; Ishikawa, K.; Mori, T. J. Mater. Chem. C 2014, 2, 9311−9317. (18) Zhang, Y.; Kim, C.; Lin, J.; Nguyen, T.-Q. Adv. Funct. Mater. 2012, 22, 97−105. (19) Katz, H. E.; Bao, Z.; Gilat, S. L. Acc. Chem. Res. 2001, 34, 359− 369. (20) Riaño, A.; Burrezo, P. M.; Mancheño, M. J.; Timalsina, A.; Smith, J.; Facchetti, A.; Marks, T. J.; Navarrete, J. T. L.; Segura, J. L.; Casado, J.; Ortiz, R. P. J. Mater. Chem. C 2014, 2, 6376−6386. (21) Zhou, K.; Dong, H.; Zhang, H.; Hu, W. Phys. Chem. Chem. Phys. 2014, 16, 22448−22457. (22) Chase, D. T.; Fix, A. G.; Kang, S. J.; Rose, B. D.; Weber, C. D.; Zhong, Y.; Zakharov, L. N.; Lonergan, M. C.; Nuckolls, C.; Haley, M. M. J. Am. Chem. Soc. 2012, 134, 10349−10352. (23) Guo, J.; Liu, D.; Zhang, J.; Zhang, J.; Miao, Q.; Xie, Z. Chem. Commun. 2015, 51, 12004−12007. (24) Ö zdemir, R.; Choi, D.; Ö zdemir, M.; Kwon, G.; Kim, H.; Sen, U.; Kim, C.; Usta, H. J. Mater. Chem. C 2017, 5, 2368−2379. (25) Zaumseil, J.; Sirringhaus, H. Chem. Rev. 2007, 107, 1296−1323. (26) Ando, S.; Nishida, J.; Tada, H.; Inoue, Y.; Tokito, S.; Yamashita, Y. J. Am. Chem. Soc. 2005, 127, 5336−5337. (27) Chen, S.; Liu, Y.; Qiu, W.; Sun, X.; Ma, Y.; Zhu, D. Chem. Mater. 2005, 17, 2208−2215. (28) Huang, J.; Fu, H.; Wu, Y.; Chen, S.; Shen, F.; Zhao, X.; Liu, Y.; Yao, J. J. Phys. Chem. C 2008, 112, 2689−2696. (29) Mishra, A.; Ma, C.-Q.; Bäuerle, P. Chem. Rev. 2009, 109, 1141− 1276. (30) Yoon, M.-H.; DiBenedetto, S. A.; Facchetti, A.; Marks, T. J. J. Am. Chem. Soc. 2005, 127, 1348−1349. (31) Balaji, G.; Kale, T. S.; Keerthi, A.; Della Pelle, A. M.; Thayumanavan, S.; Valiyaveettil, S. Org. Lett. 2011, 13, 18−21. 12501


Article

The Journal of Organic Chemistry Int. Ed. 2010, 49, 740. (n) Anthony, J. E. Chem. Mater. 2011, 23, 583− 590. (56) Geib, S.; Martens, S. C.; Märken, M.; Rybina, A.; Wadepohl, H.; Gade, L. H. Chem. - Eur. J. 2013, 19, 13811−13822. (57) Hahn, L.; Wadepohl, H.; Gade, L. H. Org. Lett. 2015, 17, 2266− 2269. (58) (a) Hahn, L.; Ö z, S.; Wadepohl, H.; Gade, L. H. Chem. Commun. 2014, 50, 4941−4943. (b) Hahn, L.; Buurma, N. J.; Gade, L. H. Chem. - Eur. J. 2016, 22, 6314−6322. (59) Martens, S. C.; Zschieschang, U.; Wadepohl, H.; Klauk, H.; Gade, L. H. Chem. - Eur. J. 2012, 18, 3498−3509. (60) Geib, S.; Zschieschang, U.; Gsänger, M.; Stolte, M.; Würthner, F.; Wadepohl, H.; Klauk, H.; Gade, L. H. Adv. Funct. Mater. 2013, 23, 3866−3874. (61) Hahn, L.; Maaß, F.; Bleith, T.; Zschieschang, U.; Wadepohl, H.; Klauk, H.; Tegeder, P.; Gade, L. H. Chem. - Eur. J. 2015, 21, 17691− 17700. (62) Pati, P. B.; Zade, S. S. Cryst. Growth Des. 2014, 14, 1695−1700. (63) Appleton, A. L.; Miao, S.; Brombosz, S. M.; Berger, N. J.; Barlow, S.; Marder, S. R.; Lawrence, B. M.; Hardcastle, K. I.; Bunz, U. H. F. Org. Lett. 2009, 11, 5222−5225. (64) Becke, A. D. J. Chem. Phys. 1993, 98, 1372−1377. (65) Becke, A. D. J. Chem. Phys. 1993, 98, 5648−5652. (66) Lee, C.; Yang, W.; Parr, R. G. Phys. Rev. B: Condens. Matter Mater. Phys. 1988, 37, 785−789. (67) Weigend, F.; Häser, M.; Patzelt, H.; Ahlrichs, R. Chem. Phys. Lett. 1998, 294, 143−152. (68) Weigend, F.; Ahlrichs, R. Phys. Chem. Chem. Phys. 2005, 7, 3297−3305. (69) Ma, C.-Q.; Mena-Osteritz, E.; Debaerdemaeker, T.; Wienk, M. M.; Janssen, R. A.; Bäuerle, P. Angew. Chem., Int. Ed. 2007, 46, 1679− 1683. (70) Seixas de Melo, J.; Burrows, H. D.; Svensson, M.; Andersson, M. R.; Monkman, A. P. J. Chem. Phys. 2003, 118, 1550−1556.

12502


(Oligo-)Thiophene Functionalized Tetraazaperopyrenes: Donor

Recommend Documents